This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Step 1: Determine the volume of the pipette used. The instructions state that a "20.00 cm^3 or 25.00 cm^3 portion of B" should be used. You must choose one of these standard pipette volumes for your experiment and record it. For example, if you choose a 25.00 cm^3 pipette, you would write: Volume of pipette used: 25.00 cm^3 (or 20.00 cm^3 if that was chosen) Step 2: Calculate the concentration of solution B (sodium hydroxide, NaOH). Given: Mass of NaOH = 1.00 g Volume of solution = 250 cm^3 First, calculate the molar mass of NaOH: Molar mass of NaOH = (22.99 g/mol for Na) + (16.00 g/mol for O) + (1.01 g/mol for H) Molar mass of NaOH = 40.00 g/mol Next, calculate the number of moles of NaOH: Moles of NaOH = MassMolar mass Moles of NaOH = 1.00 g40.00 g/mol Moles of NaOH = 0.0250 mol Convert the volume of solution to dm^3: Volume = 250 cm^3 × 1 dm^31000 cm^3 Volume = 0.250 dm^3 Finally, calculate the concentration of NaOH: Concentration of NaOH = MolesVolume Concentration of NaOH = 0.0250 mol0.250 dm^3 Concentration of NaOH = 0.100 mol/dm^3 Step 3: Explain how to complete Table 1.1. For each titration (Rough, 1, 2, 3), you will record the initial and final burette readings. The "Volume of A used" is then calculated for each titration using the formula: Volume of A used (cm^3) = Final burette reading (cm^3) - Initial burette reading (cm^3) The rough titration is an estimate, while titrations 1, 2, and 3 are precise measurements. You would typically use the concordant (closest) values from titrations 1, 2, and 3 to calculate an average volume of A used for subsequent calculations. Send me the next one 📸